Advertisements
Advertisements
Question
a. Explain the trends in the following properties with reference to group 16:
1 Atomic radii and ionic radii
2 Density
3 ionisation enthalpy
4 Electronegativity
b. In the electolysis of AgNO3 solution 0.7g of Ag is deposited after a certain period of time. Calulate the quantity of electricity required in coulomb. (Molar mass of Ag is 107.9g mol-1)
Solution
(a) Trends in 16-Group
(i) Atomic radii and ionic radii
Down the group atomic radii increases.
(ii) Density
Down the group density increased.
(iii) Ionization enthalpy
The Ist ionization enthapies of the elements of group 16 are unexpectedly lower, while their IInd ionization enthalpies are higher than those of the correspending element of group 15.
(iv) Electronegativity
The element of group 16 have higher value of electronegativity then the corresponding element of group 15.
(b) `"Mass of sub"=Q/96500xx"mole ratio"xx"mol mass"`
Mass of sub = 0.7 g
`"Mole ratio"=1/1`
Molar mass = 107.9
`:.0.7=Q/96500xx1xx107.9`
`Q=(0.7xx96500)/107.9`
`=67550/107.9`
=626.04
| Quantity of electricity = 626.04 C |
APPEARS IN
RELATED QUESTIONS
Give reasons: SO2 is reducing while TeO2 is an oxidising agent.
Give reasons for the following : H2Te is the strongest reducing agent amongst all the hydrides of Group 16 elements.
Give reasons for the following : Oxygen has less electron gain enthalpy with negative sign than sulphur.
List the important sources of sulphur.
Why is H2O a liquid and H2S a gas?
The HNH angle value is higher than HPH, HAsH and HSbH angles. Why? [Hint: Can be explained on the basis of sp3 hybridisation in NH3 and only s−p bonding between hydrogen and other elements of the group].
Justify the placement of O, S, Se, Te and Po in the same group of the periodic table in terms of electronic configuration, oxidation state and hydride formation.
Knowing the electron gain enthalpy values for O → O− and O → O2− as −141 and 702 kJ mol−1 respectively, how can you account for the formation of a large number of oxides having O2− species and not O−? (Hint: Consider lattice energy factor in the formation of compounds).
Draw the structures of `H_3PO_2`
Explain the following properties of group 16 elements :
1) Electro negativity
2) Melting and boiling points
3) Metallic character
4) Allotropy
Give reactions for the following:
O – O single bond is weaker than S – S single bond.
Give a reason for the following:
Fluorine gives only one oxide but chlorine gives a series of oxides.
The formation of \[\ce{O^+_2[PtF6]^-}\] is the basis for the formation of first xenon compound. This is because ____________.
Which of the following statement is incorrect?
Match the items of Columns I and II and mark the correct option.
| Column I | Column II |
| (A) \[\ce{H2SO4}\] | (1) Highest electron gain enthalpy |
| (B) \[\ce{CCl3NO2}\] | (2) Chalcogen |
| (C) \[\ce{Cl2}\] | (3) Tear gas |
| (D) Sulphur | (4) Storage batteries |
Given below are two statements labelled as Assertion (A) and Reason (R).
Assertion (A): Electron gain enthalpy of oxygen is less than that of Flourine but greater than Nitrogen.
Reason (R): Ionisation enthalpies of the elements follow the order Nitrogen > Oxygen > Fluorine.
Select the most appropriate answer from the options given below:
Write a balanced chemical equation for the reaction showing catalytic oxidation of NH3 by atmospheric oxygen.
Out of \[\ce{H2O}\] and \[\ce{H2S}\], which one has higher bond angle and why?
The correct order of ΔiHs among the following elements is
Which of the following compound is a peroxide?
These are physical properties of an elements.
- Sublimation enthalpy
- Ionisation enthalpy
- Hydration enthalpy
- Electron gain enthalpy
The total number of above properties that affect the reduction potential is ______. (Integer answer)
______ is a radioactive element in group 16 elements.
